Exam 2 Lecture 9/25

-prediction of how matter should behave -all mater is made up of moving particles -phase changes occur with increases in kinetic energy (typically heat)

stored energy (top of rollercoaster)

energy in motion (rollercoaster coming down)

-Physical properties of gases are similar -composed of nonmetallic elements (simple formulas, low molar masses) -gases expand to fill container, very compressible -two or more gases are homogeneous mixture

-combined volume of all molecules of the gas is negligible relative to total volume in which gas is contained -attractive/repulsive forces between gas molecules are weak -kinetic energy of gas is dependent on temperature

-temperature is related to the average kinetic energy -individual molecules can have different speeds

at any given temp, average kinetic energy is the same

gas constant 0.08206 L atm/mol K

Temperature C+ 273.15 = K

given in atmosphere (atm) 1 atm = 760 mmHg; 1 atm = 760 torr; 1 atm = 1.01325 bar; 1 atm = 101,325 Pa; 1 atm = 101.325 kPa

amount of force applied to an area

pressure of a gas is inversely related to its volume when temp is constant P1V1 = P2V2

temp of a gas is directly related to volume when pressure and amount are constant V1/T1=V2/T2

pressure exerted by a gas is directly related to the temperature of the gas when volume and amount of gas are constant P1/T1=P2/T2

combine Boyles, Charles, gay-lussac

volume of gas is directly related to amount of gas when temp and pressure are constant V1/n1=V2/n2

standard temp and pressure 1atm, 273K (one mole of gas occupies 22.4L)

PV=nRT

total pressure of a mixture of gases equal the sum of pressures from each gas

moles of compound/ total moles

relates molar mass of two gases to their rate of speed of travel

diffusion across a membrane

solubility of a gas in a given volume of liquid is directly proportional to the partial pressure of that gas in equilibrium

the ideal gas law can be adjusted to take deviations from ideal behavior into account